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zalisa [80]
4 years ago
7

Write a balanced equation and a net ionic equation for combining 2AgNO3(aq) and H2SO4(aq)

Chemistry
1 answer:
wariber [46]4 years ago
4 0
Net ionic: 2Ag+(aq) + SO4(aq) --> Ag2SO4(s)
balanced: 2 AgNO3(aq) + H2So4(aq) —> Ag2SO4(s) + 2 HNO3(aq)
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47/3 which could be simplified to 15.6
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Extreme temperature changes or increased moisture speed up the weathering rate.
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that is a true statement

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What is a chemical change
antiseptic1488 [7]

Answer:

chimical change means when one or more new substances are formed.

Explanation:

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4 years ago
Tellurium has eight isotopes: Te-120 (0.09%), Te-122 (2.46%), Te-123 (0.87%), Te-124 (4.61%), Te-125 (6.99%), Te-126 (18.71%), T
Elena-2011 [213]

The average atomic mass of tellurium, calculated from its eight isotopes (Te-120 (0.09%), Te-122 (2.46%), Te-123 (0.87%), Te-124 (4.61%), Te-125 (6.99%), Te-126 (18.71%), Te-128 (31.79%), and Te-130 (34.48%)) is 127.723 amu.

The average atomic mass of Te can be calculated as follows:

A = m_{Te-120}\%_{Te-120} + m_{Te-122}\%_{Te-122} + m_{Te-123}\%_{Te-123} + m_{Te-124}\%_{Te-124} + m_{Te-125}\%_{Te-125} + m_{Te-126}\%_{Te-126} + m_{Te-128}\%_{Te-128} + m_{Te-130}\%_{Te-130}

Where:

m: is the mass

%: is the abundance percent

Knowing all the masses and abundance values, we have:

A = 120*0.09\% + 122*2.46\% + 123*0.87\% + 124*4.61\% + 125*6.99\% + 126*18.71\% + 128*31.79\% + 130*34.48\%

To find the <u>average atomic mass</u> we need to change all the <u>percent values</u> to <u>decimal ones</u>

A = 120*9 \cdot 10^{-4} + 122*2.46 \cdot 10^{-2} + 123*8.7\cdot 10^{-3} + 124*4.61 \cdot 10^{-2} + 125*6.99\cdot 10^{-2} + 126*0.1871 + 128*0.3179 + 130*0.3448 = 127.723

Therefore, the average atomic mass of tellurium is 127.723 amu.

You can find more about average atomic mass here brainly.com/question/11096711?referrer=searchResults

I hope it helps you!

4 0
3 years ago
Solving stoichiometry problems that involve mass Now that you know the molar masses of the relevant compounds, you are ready to
Shalnov [3]

14.85 g of water

Explanation:

Calculate the mass of water produced when 9.56 g of butane reacts with excess oxygen.

Here we have the full oxidation of butane (C₄H₁₀) which produce carbon dioxide and water.

C₄H₁₀ + (13/2) O₂ → 4 CO₂ + 5 H₂O

number of moles = mass / molecular weight

number of moles of butane = 9.56 / 58 = 0.165 moles

Now, taking in account the chemical reaction, we devise the following reasoning:

if         1 mole of butane produces 5 moles of water

then    0.165 moles of butane produces X moles of water

X = (0.165 × 5) / 1 = 0.825 moles of water

mass = number of moles × molecular weight

mass of water = 0.825 × 18 = 14.85 g

Learn more about:

oxidation of hydrocarbons

brainly.com/question/10195442

brainly.com/question/7295137

#learnwithBrainly

4 0
3 years ago
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